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(A) The general combustion reaction for a hydrocarbon $C_xH_y$ is given by:$C_xH_y + (x + \frac{y}{4}) O_2 \rightarrow xCO_2 + \frac{y}{2} H_2O$Given

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$C_9H_8$

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(A) The general combustion reaction for a hydrocarbon $C_xH_y$ is given by:$C_xH_y + (x + \frac{y}{4}) O_2 \rightarrow xCO_2 + \frac{y}{2} H_2O$Given that the reaction produces $4$ equivalents of water:$\frac{y}{2} = 4 \implies y = 8$Given that the reaction requires $11$ equivalents of oxygen:$x + \frac{y}{4} = 11$Substituting $y = 8$:$x + \frac{8}{4} = 11$$x + 2 = 11$$x = 9$Therefore,the molecular formula of the hydrocarbon $A$ is $C_9H_8$.

When a hydrocarbon $A$ undergoes complete combustion,it requires $11$ equivalents of oxygen and produces $4$ equivalents of water. What is the molecular formula of $A$?

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